A 1.24 M aqueous solution of KI has density of $1.15 g / c m^{3}$ . What is the percentage composition of solute in the solution?

17.89

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

27.89

No worries! We‘ve got your back. Try BYJU‘S free classes today!

37.89

No worries! We‘ve got your back. Try BYJU‘S free classes today!

47.89

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

Solution

The correct option is A $17.89$
1.24 M aqueous solution of KI means 1.24 moles of KI in 1 litre of solution.

Given,
Density of solution $= 1.15 \frac{g}{c m^{3}}$

Volume of solution $= 1 L o r 1000 c m^{3}$

$∴$ Mass of solution $= D e n s i t y \times v o l u m e$

$= 1.15 \times 1000$

$= 1150 g$

Mass of solute $= 1.24 \times 166 = 205.8 g$

Percentage composition of solute $= \frac{Mass of solute}{Mass of solution} \times 100$

$= \frac{205.8}{1150} \times 100$

$= 17.89 %$

Hence, option A is correct.

Suggest Corrections

Similar questions

Q. A

1.24 M

aqueous solution of KI has a density of

1.15 g c m^{- 3}

What is the freezing point of the solution if the KI is completely dissociated in the solution?

Q. An aqueous solution of urea containing 18g urea in 15

c m^{3}

of the solution has a density equal to 1.052

g / c m^{3}

. If the molecular weight of urea is 60, then the molality of the solution is:

A 0.1 (M) solution of an acid HA of density 1.01 gm/ml is taken in a beaker. The molecular mass of HA is 300 $g / m o l$ . The freezing point of solution is $0.2087^{o} C$ . For $H_{2} O$ , $K_{f} = 1.86 K / m$

What is the degree of dissociation of HA in its 0.1(M) aqueous solution (in percentage) ?

Q. The percentage composition by weight of an aqueous solution of a solute (molar mass 150) which boils at 373.26 is:

(G i v e n : K_{b}

= 0.52)

Q. An aqueous solution of ethanol has a density of

1.025 g / m L

and concentration

2 M

. What is the molality of this solution?

Join BYJU'S Learning Program

A 1.24 M aqueous solution of KI has density of 1.15g/cm3 . What is the percentage composition of solute in the solution?

A 1.24 M aqueous solution of KI has density of $1.15 g / c m^{3}$ . What is the percentage composition of solute in the solution?